Answer:
22.656 grams of oxygen gas are there in a 2.3L tank at 7.5 atm and 24° C
Explanation:
An ideal gas is characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them constitutes the ideal gas law:
P * V = n * R * T
where R is the molar constant of the gases and n the number of moles.
In this case you know:
- R= 0.082
- T= 24 °C= 297 °K (being 0°C=273°K)
Replacing:
Solving:
n=0.708 moles
Knowing that oxygen gas is a diatomic gas of molecular form O₂ and its mass is 32 g / mole, you can apply the following rule of three: if 1 mole contains 32 grams, 0.708 moles, how much mass will it have?
mass= 22.656 grams
<u><em>22.656 grams of oxygen gas are there in a 2.3L tank at 7.5 atm and 24° C</em></u>
Endothermic reactions absorb heat and exothermic reactions give off heat
Answer:
Volume of the concentrated solution, which is needed is 103.30 mL
Explanation:
Let's apply the formula for dilutions to solve the problem
Conc. Molarity . Conc. volume = Dil. Molarity . Dil volume
12.1 M . Conc. volume = 2.5 M . 500 mL
Conc. volume = (2.5 M . 500 mL) / 12.1M
Conc. volume = 103.30 mL
Answer:
The third line
Explanation:
The first one us wrong because they're not all found inside,electron is outside.
The second one is wrong as I explained previously.
Lastly the fourth line is wrong because protons are found in the nucleus.
Answer:
[H₂] = 1.61x10⁻³ M
Explanation:
2H₂S(g) ⇋ 2H₂(g) + S₂(g)
Kc = 9.30x10⁻⁸ = ![\frac{[H_{2}]^2[S_{2}]}{[H_{2}S]^2}](https://tex.z-dn.net/?f=%5Cfrac%7B%5BH_%7B2%7D%5D%5E2%5BS_%7B2%7D%5D%7D%7B%5BH_%7B2%7DS%5D%5E2%7D)
First we <u>calculate the initial concentration</u>:
0.45 molH₂S / 3.0L = 0.15 M
The concentrations at equilibrium would be:
[H₂S] = 0.15 - 2x
[H₂] = 2x
[S₂] = x
We <u>put the data in the Kc expression and solve for x</u>:
We make a simplification because x<<< 0.0225:
x = 8.058x10⁻⁴
[H₂] = 2*x = 1.61x10⁻³ M
